Question

A voltaic cell employs the following redox reaction:

( Sn²+(aq) + Mn(s) longrightarrow Sn(s) + Mn²+(aq) )
Calculate the cell potential, in volts, at 25°C under standard conditions.
a) +2.71 V
b) -2.71 V
c) +1.36 V
d) -1.36 V

Answer 1

The cell potential of the voltaic cell is -1.04 V, which is not provided in the given options.

Step-by-step explanation:

The cell potential of a voltaic cell can be calculated using the standard reduction potentials of the half-cell reactions involved. In this case, the reduction half-reaction is Mn²+(aq) + 2e- → Mn(s) with a standard reduction potential of -1.18 V, and the oxidation half-reaction is Sn(s) → Sn²+(aq) + 2e- with a standard reduction potential of -0.14 V. To calculate the cell potential, we subtract the reduction potential of the anode (oxidation half-reaction) from the reduction potential of the cathode (reduction half-reaction):

Cell potential = reduction potential of cathode - reduction potential of anode

Cell potential = (-1.18 V) - (-0.14 V) = -1.04 V

Since the given options do not match with the calculated cell potential, none of the provided options are correct. Therefore, the correct answer is not provided in the given options.